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Quiz 12.82 In a mountainous location. the boiling point of pure wa- ter is found to...
F. A solution was prepared by dissolving 0.800 g of sulfur S8, in 100.0 g of...
F. A solution was prepared by dissolving 0.800 g of sulfur S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution . For the solvent, Kb = 3.08 oC/m and Kf = 3.59 oC/m. G. Butylated hydroxytoluene (BHT) is used as an antioxidant in processed foods. (It prevents fats and oils from becoming rancid.) A solution of 2.500 g of BHT in 100.0 g of benzene had a freezing point of...
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of zinc chloride...
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of zinc chloride (136.3 g/mol), must be dissolved in 209.0 grams of water to raise the boiling point by 0.400°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g zinc chloride.
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezin...
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C....
You want to raise the boiling point of 1.00 L of water by 2.70 °C by...
You want to raise the boiling point of 1.00 L of water by 2.70 °C by adding some sodium chloride. How much sodium chloride would you need to add to achieve such an increase in boiling point? [Kb(H2O) = 0.710 °C/m)] a) 1.90 g b) 22.4 g c) 111 g d) 222 g e) 4227 g Answer is c) - can you explain this? I found d) again and again....
1) At physiological temperature (37OC) the osmotic pressure of blood is 7.65 atm. What concentration (%...
1) At physiological temperature (37OC) the osmotic pressure of blood is 7.65 atm. What concentration (% W/V) of potassium chloride (KCl, MW = 74.5) solution has the same osmotic pressure of blood? Assume the specific gravity of the solution is 1. 2)An ophthalmic (eye drop) formulation contains 100 mEq of sodium chloride (molecular weight = 58.5 g/mole). Calculate the amount (in grams) of sodium chloride needed for the formulation. 3)Methanol (CH3OH, MW = 32) is a nonelectrolyte. What is the...
two Part question A: The boiling point of water is 100.0°C at 1 atmosphere. How many...
two Part question A: The boiling point of water is 100.0°C at 1 atmosphere. How many grams of chromium(II) bromide (211.8 g/mol), must be dissolved in 287.0 grams of water to raise the boiling point by 0.400°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g chromium(II) bromide. ____ ? B...
1. Why does freezing point vary with different salts? 2. What does % ionization mean? Why...
1. Why does freezing point vary with different salts? 2. What does % ionization mean? Why should it be less than 100%? 3. Should the percent ionization be closer to ideal at high or low concentrations? 4. As you increase elevation the atmospheric pressure decreases, which means the boiling point of water also decreases. In Denver, the boiling point of water is 95 degrees C. - 4a. How many grams of NH4Cl (using van't Hoff factor of 1.699) would need...
How many grams of ice at -15°C must be added to 705 grams of water that...
How many grams of ice at -15°C must be added to 705 grams of water that is initially at a temperature of 88°C to produce water at a final temperature of 11°C. Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg·C° and of ice is 2050 J/kg·C°. For water the normal melting point is 0.00°C and the heat of fusion is 334 × 103...
*Please explain answers* Sodium chloride (MW 58.5) is often used in road and sidewalk treatment during the winter to pr...
*Please explain answers*
Sodium chloride (MW 58.5) is often used in road and sidewalk treatment during the winter to prevent ice formation. How many grams of sodium chloride should be added to 0.5 kg of water to lower the freezing point by 3°C? The cryoscopic constant of water is 1.860 deg-kg/mole. Calculate the molality of a of 20% solution of a nonelectrolyte (MW = 300). Assume the density of the solution is 1.0. Please provide the value ofi (van't hoff...
Enter your answer in the provided box. The formula that governs the depression of freezing point...
Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: where:AT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions, i = 2 for...
*Please explain answers*
Sodium chloride (MW 58.5) is often used in road and sidewalk treatment during the winter to prevent ice formation. How many grams of sodium chloride should be added to 0.5 kg of water to lower the freezing point by 3°C? The cryoscopic constant of water is 1.860 deg-kg/mole. Calculate the molality of a of 20% solution of a nonelectrolyte (MW = 300). Assume the density of the solution is 1.0. Please provide the value ofi (van't hoff...
Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: where:AT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions, i = 2 for...
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